Draw Lewis dot structures for the following compounds: NaCl, CaF₂, H₂, O₂, N₂.

Here are the Lewis dot formulae for the bond formations in the given compounds:

a) NaCl (Sodium Chloride)
Sodium (Na) has 1 valence electron, and Chlorine (Cl) has 7 valence electrons. Sodium transfers its electron to chlorine, forming an ionic bond.

$$\text{Na} \cdot + \cdot \ddot{\text{Cl}}: \longrightarrow \text{Na}^{+} [: \ddot{\text{Cl}}:]^{-}$$

b) CaF₂ (Calcium Fluoride)
Calcium (Ca) has 2 valence electrons, and each Fluorine (F) has 7 valence electrons. Calcium transfers one electron to each of the two fluorine atoms, forming ionic bonds.

$$\cdot \text{Ca} \cdot + 2 \cdot \ddot{\text{F}}: \longrightarrow \text{Ca}^{2+} 2[: \ddot{\text{F}}:]^{-}$$

c) H₂ (Hydrogen molecule)
Each Hydrogen (H) atom has 1 valence electron. They share their electrons to form a single covalent bond.

$$\text{H} \cdot + \cdot \text{H} \longrightarrow \text{H} : \text{H}$$

d) O₂ (Oxygen molecule)
Each Oxygen (O) atom has 6 valence electrons. They share two pairs of electrons to form a double covalent bond, and each oxygen atom has two lone pairs.

$$: \ddot{\text{O}} \cdot + \cdot \ddot{\text{O}}: \longrightarrow : \ddot{\text{O}} :: \ddot{\text{O}}:$$

e) N₂ (Nitrogen molecule)
Each Nitrogen (N) atom has 5 valence electrons. They share three pairs of electrons to form a triple covalent bond, and each nitrogen atom has one lone pair.

$$\cdot \ddot{\text{N}} \cdot + \cdot \ddot{\text{N}} \cdot \longrightarrow : \text{N} ::: \text{N}:$$

f) H₂O (Water molecule)
Oxygen (O) has 6 valence electrons, and each Hydrogen (H) has 1 valence electron. Oxygen forms a single covalent bond with each hydrogen atom and has two lone pairs.

$$\text{H} \cdot + \cdot \ddot{\text{O}} \cdot + \cdot \text{H} \longrightarrow \text{H} : \ddot{\text{O}} : \text{H}$$